organometallic compounds iiorganometallic compounds ii (part ii) b.sc. (h) chemistry dr. rajanish n....
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Organometallic Compounds II(Part II)
B.Sc. (H) Chemistry
Dr. Rajanish N. TiwariDepartment of ChemistryMahatma Gandhi Central University
UNIT III
Infrared Spectra for organometallic compounds
The carbonyl group in organometallic compounds are
used to study by Infrared spectroscopy.
The position of the Infrared band can indicate the function of a
ligand (e.g., terminal vs. bridging modes).
In the case of π –acceptor ligands, can describe the electronic
environment of the metal.The peak appear in the range between 2100-1700 cm-1
Number of Infrared Bands
A molecular vibration is infrared active (i.e., excitation of
the vibrational mode can be measured via an IR spectrum
absorption) only if it results in a change in the dipole
moment of the molecule
It is often useful to consider a particular vibrational mode for a
compound.
For example, useful information often can be obtained from the
C-O stretching bands in infrared spectra of metal complexes
containing CO (carbonyl) ligands.
Selected Vibrational Modes
These complexes have a single C-O stretching mode
and consequently show a single band in the IR.
Monocarbonyl Complexes
Dicarbonyl Complexes
Two geometries, linear and bent, must be considered:
O – C – M – C – O
Two CO ligands arranged linearly, Only an antisymmetric vibration of theligands is IR active
Two CO ligands are oriented in a nonlinear fashion, both symmetric and
antisymmetric vibrations result in changes in dipole moment, and both are IR
active:
Two CO ligands are oriented in a nonlinear fashion, both symmetric and
antisymmetric vibrations result in changes in dipole moment, and both
are IR active:
Symmetric Stretch
Antisymmetric Stretch
Continue..
IR spectrum is a convenient tool for determining the structure of
molecules with two CO ligands: a single band indicates linear
orientation of the CO ligands, and two bands indicate nonlinear
orientation.
Continue..
For molecules containing two CO ligands on the same metal atom, the
relative intensities of the IR bands can be used to determine the
approximate angle between the CO ligands, using the equation
Where φ is the angle between ligands
Continue..
Complexes containing three or more carbonyls
The predictions for the Complexes containing three or more carbonyls
are not quite so simple.
The exact number of carbonyl bands can be determined according to the
symmetry approach. (not discussed here).
In carbonyl complexes, the number of C-O stretching bands cannot
exceed the number of CO ligands.
The alternative is possible in some cases (more CO groups than IR
bands), when vibrational modes are not IR active (do not cause a change in
dipole moment).
For convenient reference, the numbers of bands expected for a variety of COcomplexes are given in next slide.
Carbonyl stretching bands
Carbonyl stretching bands
Positions of IR Bands
The position of the carbonyl stretching band always provides usefulinformation.
In the case of the isoelectronic species [Mn(CO)6]+, Cr(CO)6, and [V(CO)6]-, anincrease in negative charge on the complex causes a significant reduction inthe energy of the C-O band as a consequence of additional π back-bondingfrom the metal to the ligands.
The bonding mode is also reflected in the infrared spectrum, with energy decreasing in the order
terminal CO > doubly bridging CO > triply bridging CO
The position of the carbonyl bands provide important clues to the electronic
environment of the metal.
The greater the electron density on the metal (and the greater the negative
charge), the greater the back-bonding to CO, and the lower the energy of the
carbonyl stretching vibrations.
The positions of infrared bands are also a function of other ligands present.
Continue..
References:
(1) Miessler, Fischer & Tarr Inorganic Chemistry
(2) Shriver & Atkins Inorganic Chemistry
Thank You